Give the representation for the cell with cell reaction as:

$2\mathrm{Al}+3{\mathrm{Zn}}^{2+}⟶2{\mathrm{Al}}^{3+}+3\mathrm{Zn}$

A conventional method of representing Daniell cell is:

$Zn\left(\mathrm{s}\right)\overline{)} {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)\left(1\mathrm{M}\right)\Vert {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)\left(1\mathrm{M}\right)\overline{)}; Cu\left(\mathrm{s}\right)$

Draw a diagram of the cell and mark anode and cathode.

${\mathrm{Cu}}^{2+}/\mathrm{Cu}=0.34 \mathrm{V}; {\mathrm{Zn}}^{2+}/\mathrm{Zn}=-0.76 \mathrm{V}$

A conventional method of representing Daniell cell is:

$Zn\left(\mathrm{s}\right); {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)\left(1\mathrm{M}\right)\Vert {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)\left(1\mathrm{M}\right); Cu\left(\mathrm{s}\right)$

Give the net reaction as current is drawn.

A conventional method of representing Daniell cell is:

$Zn\left(\mathrm{s}\right); {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)\left(1\mathrm{M}\right)\Vert {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)\left(1\mathrm{M}\right); Cu\left(\mathrm{s}\right)$

${\mathrm{Cu}}^{2+}/\mathrm{Cu}=0.34 \mathrm{V}; {\mathrm{Zn}}^{2+}/\mathrm{Zn}=-0.76 \mathrm{V}$

What is the cell potential at $298 \mathrm{K}?$

Calculate the voltage of following electrochemical cell under standard conditions. Name anode and cathode in each cell.

$\mathrm{Zn}-\mathrm{Ag}$

The standard reduction potentials of various half-cells are:

${\mathrm{Zn}}^{2+}/\mathrm{Zn}=-0.76 \mathrm{V}; {\mathrm{Ag}}^{+}/\mathrm{Ag}=+0.80 \mathrm{V}$

Calculate the voltage of following electrochemical cell under standard conditions. Name anode and cathode in each cell.

$\mathrm{Co}-\mathrm{Ni}$

The standard reduction potentials of various half-cells are:

${\mathrm{Co}}^{2+}/\mathrm{Co}=-0.28 \mathrm{V}; {\mathrm{Ni}}^{2+}/\mathrm{Ni}=-0.25 \mathrm{V}$

Predict the possibility of occurrence of the following reactions:

$\mathrm{Zn}+2{\mathrm{H}}^{+}⟶{\mathrm{Zn}}^{2+}+{\mathrm{H}}_2$

Predict the possibility of occurrence of the following reactions:

$2\mathrm{Ag}+2{\mathrm{H}}^{+}⟶2{\mathrm{Ag}}^{+}+{\mathrm{H}}_2$